Standard Cell Potential & the Equilibrium Constant

Concept #1: Once a chemical reaction reaches equilibrium connections between the standard cell potential, Gibbs Free Energy and the equilibrium constant can be made. 

Example #1: Determine the equilibrium constant K for the following reaction:

 Au⁺ (aq) + Ce (s)  ⇌  Ce³⁺ (aq) + Au (s)               

The half reactions are determined as:

Au⁺ (aq) + e ^–  ⇌  Au (s)      E^o = 1.690 V                     

Ce³⁺ (aq) + 3 e ^–  ⇌  Ce (s)     E^o​ = -2.336 V                

Example #2: From the two half reactions provided the equilibrium constant is calculated as 6.79 x 10³⁰.

ClO (g)  +  e^– ⇌  ClO^– (g)   E^o = ?

Bi (s)  ⇌  Bi³⁺ (aq)  +  3 e^–   E^o = 0.308 V

Determine the standard cell potential for:

ClO (g)  +  e^– ⇌  ClO^– (g)   E^o = ?